Finding salt concentrations :

can someone please help me with this problem, its giving me lots of trouble to solve :

(a) Suppose you wanted to make a buffer of exactly ph 7.00 using KH2PO4 and Na2HPO4. If you had a solution of 0.1M KH2PO4, what concentration of Na2HPO4 would you need?

(b)Now assume you wish to make a buffer at the same ph, using the same substances, but want the total phosphate molarity (HPO42-) + (H2PO4-) to equal 0.3 What concentrations of KH2PO4 and Na2HPO4 would you use?

If you want to find pH, then you should use pKa of the acid in Henderson-Hasselbach equation.
In your second question, you don't know the molar ratio of conjugate base to acid. The rest is known, just find it.

Yes that's correct, but it is invalid for this question, as phosphate species other than ortho-phosphoric acid (H3PO4) need pKa values. If you were not given that data, it is nearly not possible to solve the H-H equation. Please find the pKa values for them, and solve this question. It is not that difficult. But when you think you're lost, keep asking.

I was given this lab problem calc the ph values and draw the titration curve for the titration of 500ml of 0.010m acetic acid (pka 4.76) with .010m KOH.
I have to give two points the starting ph and the equivalence point.

I found the equivalence point to be the pka ( where ph=pka ).
I know i have to calc the second point using the KA Im just not sure how to plot the x-axis and y-axis

for the y-axis i know i have to plot ph
but for the x-axis is it KOH (eq ) or what ?
im not sure
can someone help me with this one ?

Well, the starting pH will be the pH of the acetic acid solution with no KOH added, I am sure you are not asking this. What you're asking instead is simple, too; just plot the curve between titer (mL of KOH solution) and pH, on x and y axis, respectively.